US5858573A - Chemical overcharge protection of lithium and lithium-ion secondary batteries - Google Patents
Chemical overcharge protection of lithium and lithium-ion secondary batteries Download PDFInfo
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- US5858573A US5858573A US08/703,577 US70357796A US5858573A US 5858573 A US5858573 A US 5858573A US 70357796 A US70357796 A US 70357796A US 5858573 A US5858573 A US 5858573A
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/056—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes
- H01M10/0564—Accumulators with non-aqueous electrolyte characterised by the materials used as electrolytes, e.g. mixed inorganic/organic electrolytes the electrolyte being constituted of organic materials only
- H01M10/0566—Liquid materials
- H01M10/0567—Liquid materials characterised by the additives
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/42—Methods or arrangements for servicing or maintenance of secondary cells or secondary half-cells
- H01M10/4235—Safety or regulating additives or arrangements in electrodes, separators or electrolyte
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M10/00—Secondary cells; Manufacture thereof
- H01M10/05—Accumulators with non-aqueous electrolyte
- H01M10/052—Li-accumulators
- H01M10/0525—Rocking-chair batteries, i.e. batteries with lithium insertion or intercalation in both electrodes; Lithium-ion batteries
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M4/00—Electrodes
- H01M4/02—Electrodes composed of, or comprising, active material
- H01M4/36—Selection of substances as active materials, active masses, active liquids
- H01M4/58—Selection of substances as active materials, active masses, active liquids of inorganic compounds other than oxides or hydroxides, e.g. sulfides, selenides, tellurides, halogenides or LiCoFy; of polyanionic structures, e.g. phosphates, silicates or borates
- H01M4/583—Carbonaceous material, e.g. graphite-intercalation compounds or CFx
- H01M4/587—Carbonaceous material, e.g. graphite-intercalation compounds or CFx for inserting or intercalating light metals
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M50/00—Constructional details or processes of manufacture of the non-active parts of electrochemical cells other than fuel cells, e.g. hybrid cells
- H01M50/50—Current conducting connections for cells or batteries
- H01M50/572—Means for preventing undesired use or discharge
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M6/00—Primary cells; Manufacture thereof
- H01M6/14—Cells with non-aqueous electrolyte
- H01M6/16—Cells with non-aqueous electrolyte with organic electrolyte
- H01M6/162—Cells with non-aqueous electrolyte with organic electrolyte characterised by the electrolyte
- H01M6/168—Cells with non-aqueous electrolyte with organic electrolyte characterised by the electrolyte by additives
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- H—ELECTRICITY
- H01—ELECTRIC ELEMENTS
- H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
- H01M6/00—Primary cells; Manufacture thereof
- H01M6/14—Cells with non-aqueous electrolyte
- H01M6/18—Cells with non-aqueous electrolyte with solid electrolyte
- H01M6/181—Cells with non-aqueous electrolyte with solid electrolyte with polymeric electrolytes
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- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
- Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
- Y02E60/10—Energy storage using batteries
-
- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y10—TECHNICAL SUBJECTS COVERED BY FORMER USPC
- Y10T—TECHNICAL SUBJECTS COVERED BY FORMER US CLASSIFICATION
- Y10T29/00—Metal working
- Y10T29/49—Method of mechanical manufacture
- Y10T29/49002—Electrical device making
- Y10T29/49108—Electric battery cell making
Definitions
- This invention relates to electrochemical cells and more particularly to improved non-aqueous liquid and polymer electrolytes for cells incorporating alkali metal negative electrodes (anodes), and especially lithium anodes or lithium-ion anodes.
- the improvement features the use of a new class of compounds as redox reagents, dissolved in non-aqueous electrolytes, to provide overcharge protection.
- the electrolyte solution is a crucial component in an ambient temperature secondary lithium cell.
- a non-aqueous solvent or mixture of solvents which dissolves an appreciable amount of lithium salts to form highly conducting solutions is desirable.
- the electrolyte should afford high efficiency for cycling of the lithium or lithium-ion electrode, and exhibit good thermal stability up to 70° C. (the usual upper temperature limit for operation of ambient temperature batteries).
- a highly desirable liquid electrolyte solution established for ambient temperature Li secondary cells is described in U.S. Pat. No. 4,489,145. It comprises a solution of LiAsF 6 dissolved in a mixed solvent of tetrahydrofuran (THF), 2-methyltetrahydrofuran (2-Me-THF), and 2-methylfuran (2-Me-F).
- THF tetrahydrofuran
- 2-Me-THF 2-methyltetrahydrofuran
- 2-Me-F 2-methylfuran
- Other aprotic electrolytes have contained cyclic carbonates such as propylene carbonate (PC) and ethylene carbonate (EC), and have been the subject of much study in terms of both basic electrochemistry and battery applications for many years.
- PC propylene carbonate
- EC ethylene carbonate
- PAN polyacrylonitrile
- PEGDA poly(tetraethylene glycol diacrylate)
- PVP poly(vinyl) pyrrolidinone
- PVC poly (vinyl chloride)
- PVS poly(vinyl sulfone)
- the polymers are matrices to immobilize complexes (solvates) formed between Li salts, such as LiAsF 6 , LiCF 3 SO 3 , LiPF 6 , LiN(CF 3 SO 2 ) 2 and LiBF 4 , and an aprotic organic solvent (or mixture of such solvents) to allow fabrication of free-standing electrolyte films to be used in solid-state Li and Li-ion batteries (K. M. Abraham et al., U.S. Pat. Nos. 5,219,679; 5,252,413; 5,457,860).
- Li salts such as LiAsF 6 , LiCF 3 SO 3 , LiPF 6 , LiN(CF 3 SO 2 ) 2 and LiBF 4
- an aprotic organic solvent or mixture of such solvents
- non-aqueous electrolyte (organic electrolyte) cells may not be overcharged without causing irreversible electrolyte side-reactions which deteriorate cell performance.
- Cells are safeguarded during laboratory charge/discharge tests by careful control of the voltage limits by means of the electronic equipment used in the test.
- Electronic overcharge control comprises a sensing circuit which prevents current from flowing into the cell once it reaches the voltage corresponding to complete charge.
- the charge voltage limit is selected according to the electrochemical couple in the cell. For example, Carbon/LiMn 2 O 4 cells have an upper charge limit of 4.3V vs. Li + /Li.
- Chemical overcharge protection of a battery consisting of cells connected in series is particularly important for two reasons. Firstly, it will replace electronic overcharge controllers in individual cells. Electronic controllers lower the energy density of the battery and increase battery cost. Secondly, it will provide capacity balance among the individual cells and prevent oxidative degradation of the electrolyte. The capacity balance among the cells in a battery may be lost, especially after repeated charge/discharge cycles. This means that the accessible capacity of individual cells may not remain equal. In this instance, the cathode of the cell with the lowest capacity will be pushed above the normal upper voltage limit. Oxidative degradation of the electrolyte will occur at these higher potentials, and this will degrade the cycle life of the battery at an accelerated rate.
- the weaker cell will contribute a larger fraction of the total cutoff voltage for the battery causing the capacity of the cells in the battery to become increasingly out of balance at each additional cycle, since the stronger cells will not be charged to their full capacity. The result is a reduced cycle life for the battery as compared to its individual cells.
- a redox shuttle offers the best approach to cell overcharge protection.
- a material with an appropriate oxidation potential is dissolved in the electrolyte where it remains unreactive until the cell is charged fully.
- the redox shuttle is activated by its electrochemical conversion.
- the cell potential during overcharge is fixed at the oxidation potential of the redox shuttle. This process is supported by diffusion of the oxidized products to the anode where they recombine to form the starting material. Once the reformed material diffuses back to the cathode, it is oxidized and the cathode potential is maintained indefinitely at the oxidation potential of the redox reagent, until the time that charging is terminated.
- Necessary properties of a redox shuttle include: high solubility in the electrolyte; an oxidation potential slightly higher than the normal charge limit of the cell but lower than the oxidation potential of the electrolyte; the ability of the oxidized form to be reduced at the anode without side reactions; and chemical stability in the cell of both the oxidized and reduced forms of the shuttle reagent.
- an object of this invention is the use of redox reagents to provide a means of chemical overcharge protection to secondary non-aqueous liquid and polymer electrolyte cells with lithium or lithium-ion anodes.
- the invention features a rechargeable electrochemical cell which includes an anode, a cathode, and an electrolyte.
- the electrolyte is a non-aqueous solvent or a mixture of non-aqueous solvents which may or may not be immobilized in a polymer matrix, and in which one or more salts and the redox reagent are dissolved.
- the redox reagent is ideally present in an amount sufficient to maintain proper mass transport for the desired steady overcharge current for the cell.
- FIG. 1 shows the structure of thianthrene.
- FIG. 2 shows the structure of 2,7-diacetyl thianthrene.
- FIG. 3 shows the cyclic voltammogram obtained with a Li//organic electrolyte//glassy carbon cell in which the electrolyte was 50% EC:50% PC-1.0M LiPF 6 with 10 mM thianthrene.
- the scan rate was 100 mV/s.
- FIG. 4 shows the reversible extraction and insertion of lithium for LiMn 2 O 4 .
- Data were collected using a cell with the configuration Li//PAN-EC-PC-LiPF 6 //LiMn 2 O 4 and the scan rate was 20 ⁇ V/s.
- FIG. 5 shows the shift in the redox potential obtained by acetylating thianthrene to form 2,7-diacetyl thianthrene.
- the electrolyte was 50% EC:50% PC-1.0M LiPF 6 with 10 mM 2,7-diacetyl thianthrene, and the scan rate was 100 mV/s.
- FIGS. 6A and 6B show the voltage profile for charge/discharge of a Li//Solid Polymer Electrolyte//LiMn 2 O 4 cell at the first (a) and second (b) cycles.
- the charge limit was 4.2V for the first cycle.
- the charge limit was raised to 4.3V for the second cycle but did not yield significantly more capacity.
- FIG. 7 is a cyclic voltammogram for a carbon//polymer electrolyte//LiMn 2 O 4 cell containing 2,7-diacetyl thianthrene in the electrolyte and cycled at 20 ⁇ V/s.
- thianthrenes are used for the protection of lithium and lithium-ion secondary cells from the effects of overcharge. Their activity is manifested through the redox shuttle reactions depicted in Scheme I. ##STR1##
- R represents thianthrene (FIG. 1), or one of its derivatives such as 2,7-diacetyl thianthrene (FIG. 2).
- R is added to the electrolyte where it is available for a reversible oxidation-reduction (redox) shuttle reaction.
- the electrolyte may be a liquid solution with a single solvent, such as propylene carbonate-1.0M LiPF 6 , or a mixed-solvent solution such as 50% ethylene carbonate:50% propylene carbonate-1.0M LiPF 6 .
- inventions may have the liquid electrolyte immobilized into a polymer such as poly(acrylonitrile) (PAN), poly(tetraethylene glycol diacrylate) (PEGDA), polyvinyl pyrrolidinone (PVP), poly(vinyl chloride), poly(vinyl sulfone), poly(ethylene oxide) or poly(vinylidene fluoride) (PVdF) as described in the aforementioned U.S. Patents pertaining to polymer electrolytes.
- PAN poly(acrylonitrile)
- PEGDA poly(tetraethylene glycol diacrylate)
- PVP polyvinyl pyrrolidinone
- PVdF poly(vinyl chloride)
- PVdF poly(vinylidene fluoride)
- the protective redox shuttle reaction is initiated when the cathode reaches the oxidation potential of the redox reagent as in 1!. It proceeds with the diffusion of the oxidized species (R + ) to the anode where it is reformed as in 2!. The reaction is sustained by diffusion of the reformed reagent back to the cathode. Judicious selection of the particular thianthrene will allow the overcharge protection agent to be tailored to the appropriate cell voltage.
- the redox potential of prospective shuttle candidates is determined readily from cyclic voltammetry of glassy carbon microelectrodes in electrolyte containing the compound of interest. For example, a solution of 10 mM thianthrene, in 50% EC:50% PC-1.0M LiPF 6 , was tested at a scan rate of 100 mV/s.
- FIG. 3 shows a symmetrical wave which is characteristic of a reversible reaction with the peak oxidation current at 4.12V and the corresponding reduction (regeneration of the starting material) at 4.06V vs. Li + /Li.
- FIG. 4 shows that Li is removed from LiMn 2 O 4 in two stages, with peaks centered at 4.05V and at 4.17V vs.. Li + /Li. Consequently, although thianthrene exhibits the desired redox behavior, it is not suitable for use in the C/LiMn 2 O 4 cell since the activation of the redox shuttle would overlap with the removal of lithium from the cathode. This would interfere with the cathode utilization so that the cell would not charge fully.
- Table 2 shows the current function (i a p / ⁇ 1/2 , where i a is the peak current for the anodic peak and ⁇ is the scan rate) obtained for the oxidative and reductive peaks seen in the cyclic voltammogram for 2,7-diacetyl thianthrene, along with the voltages for the anodic and cathodic peaks ( a E p and c E p , respectively), the peak width ( ⁇ a E p/2 ), and the peak separation ( ⁇ a E p ).
- the redox shuttle is thianthrene (FIG. 1) or a derivative of thianthrene such as 2,7-diacetyl thianthrene (FIG. 2)
- the rechargeable cell is carbon/spinel LiMn 2 O 4 containing a nonaqueous liquid electrolyte such as ethylene carbonate/propylene carbonate-lithium salt, or a nonaqueous polymer electrolyte as described in U.S. Pat. Nos. 4,857,423; 5,219,413; 5,252,413; and 5,474,860.
- the anode may be either disordered carbon or graphite.
- the disordered carbon may be one obtained from the pyrolysis of petroleum coke, and known to those skilled in the field as ⁇ petroleum coke ⁇ or ⁇ coke ⁇ .
- the graphite may have the usual flake morphology, but may also be formed as graphite fibers or microtubules.
- the primary purpose of the acetyl functional groups of diacetyl thianthrene is to shift the redox potential to a more positive value.
- functional groups may be added to promote solubility of the derivatized compound in the electrolyte.
- Other functional groups can be attached to thianthrene to either increase or decrease its redox potential. Electron withdrawing substituents such as acetyl, nitro and chloro groups are expected to increase the oxidation potential while electron releasing substituents such as alkyl groups will decrease this potential.
- thianthrene and its derivatives such as 2,7-diacetyl thianthrene are useful as overcharge protection additives for lithium or lithium-ion cells.
- the choice of a particular redox reagent will vary with the cathode material used in a rechargeable Li or lithium-ion cell.
- the carbon/spinel LiMn 2 O 4 couple is mentioned specifically, other cathodes such as LiCoO 2 or LiNiO 2 might also be used.
- oxidation potential of the shuttle reagent be slightly higher than the full charge limit of the cell.
- oxidation of the redox reagent should take place after the full capacity of the cathode has been accessed.
- the shuttle should be activated at a potential above 4.2V vs. Li + /Li.
- acetyl groups for hydrogen atoms at the 2,7 positions in thianthrene resulted in a shift of the redox potential to values more positive than those obtained with thianthrene.
- the preferred electrolytes are resistive to oxidation in this range.
- liquid electrolytes with ethylene carbonate (EC), propylene carbonate (PC), dipropyl carbonate (DPC), methyl ethyl carbonate (MEC) and similar solvents or mixtures of solvents are known to those skilled in the art as desirable electrolytes for use with high voltage cathodes.
- these solvents or mixtures of solvents and the solvates which they form with lithium salts such as LiAsF 6 , LiPF 6 , LiClO 4 , LiN(SO 2 CF 3 ) 2 , LiC(SO 2 CF 3 ) 3 , LiBF 4 , and lithium salts of organic acids such as trichioroacetic, trifluoromethane sulfonic, and formic acids can be immobilized according to the teachings of the patents by Abraham et al. cited above.
- the example shows the usefulness of 2,7-diacetyl thianthrene in the presence of Li 1 .5 Mn 2 O 4 , which is a mixture of 0.5 mole of LiMn 2 O 4 and 0.5 mole of Li 2 Mn 2 O 4 .
- the cell used to demonstrate the invention contained a Li 1 .5 Mn 2 O 4 cathode, a solid polymer electrolyte, and a carbon counter electrode.
- the cathode composition was 93.5% Li 1 .5 Mn 2 O 4 :4% carbon black:2.5% PAN containing the liquid electrolyte 50% EC:50% PC-1.0M LiPF 6 , with 10 mM 2,7-diacetyl thianthrene.
- the carbon electrode comprised 97.5% petroleum coke:2.55 PAN and the same liquid electrolyte.
- the solid polymer electrolyte film used as a separator between the two electrodes had the composition 13.87% PAN:38.63% EC:38.63% PC:7.93% LiPF 6 :0.93% 2,7-diacetyl thianthrene.
- % stands for percent by weight.
- DAcTH 2,7-diacetyl thianthrene
- the cathode electrode was 93.5% LiMn 2 O 4 :4% carbon black:2.5% PAN, while the anode electrode was 97.5% petroleum coke:2.5% PAN.
- the current collector was aluminum foil for the cathode and copper foil for the anode. Both electrodes were dried under vacuum at room temperature for 2 hours, then hot-pressed at 130° C. and 5,000 psig for 2 min. The electrodes were trimmed to size, and a liquid electrolyte comprising 50% EC:50% PC-1.0M LiPF 6 , 10 mM 2,7-diacetyl thianthrene was added to each electrode, with the excess allowed to drain away. The cell was assembled in a metallized plastic bag which was heat-sealed at its periphery to prevent air and moisture ingression.
- FIG. 7 shows clearly the presence of the two peaks expected for the lithium extraction from LiMn 2 O 4 at 4.05 (1a, and its inverse peak 1c; where a represents the anodic peak and c represents the cathodic peak) and 4.17V (2a, 2c ) and an additional reversible peak at 4.4V (3a, 3c). These last peaks corresponds the oxidation and reduction of acetyl thianthrene.
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Abstract
Description
TABLE 1 ______________________________________ Redox Potential Ranges of Chemical Shuttle Reagents. Redox Potential Range Compound (V vs. Li.sup.+ /Li) ______________________________________ Thianthrene 4.06-4.12 2,7-diacetyl Thianthrene 4.19-4.30 ______________________________________
Peak Width=Δ.sup.a E.sub.p/2 =.sup.a E.sub.p -.sup.a E.sub.p/2 =2.20RT/nF=0.0565/n @25° C. 3!
Peak Separation=Δ.sup.a E.sub.p =.sup.a E.sub.p -.sup.c E.sub.p =2.22RT/nF=0.058/n @25°
TABLE 2 ______________________________________ Electrochemical Data for Cyclic Voltammetry of 2,7-Diacetyl Thianthrene at Different Sweep Rates. Sweep Current Anodic Cathodic Peak Peak Rate Function Peak Voltage Peak Voltage Width Separation ν i.sup.a.sub.p /ν.sup.1/2 .sup.a E.sub.p .sup.c E.sub.p Δ.sup.a E.sub.p/2 ΔE.sub.p (V/s) A/(V/s).sup.1/2 (V) (V) (V) (V) ______________________________________ 0.001 1.897 × 10.sup.-4 4.255 4.205 0.055 0.050 0.005 1.824 × 10.sup.-4 4.258 4.200 0.053 0.058 0.010 1.820 × 10.sup.-4 4.260 4.200 0.055 0.060 0.020 1.789 × 10.sup.-4 4.260 4.200 0.055 0.060 0.050 1.766 × 10.sup.-4 4.260 4.200 0.055 0.060 ______________________________________
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